1. Net Ionic Equations Unit 5 – Lesson 4
Demos
It is Eggothermic

2. NaCl(s)  Na+(aq) + Cl-(aq)
Dissolution
Dissolution is the process by which an ionic solid dissolves in a polar liquid, such as water.
We can write these solutions as ions if they dissolve (aqueous)
NaCl(s)  Na+(aq) + Cl-(aq)

4. Ag+(aq) + Cl-(aq)  AgCl(s)
Precipitation
Precipitation is the process in which ions leave a solution and form a precipitate.
It is the opposite of dissolution.
Ag+(aq) + Cl-(aq)  AgCl(s)

5. Net Ionic Equations X X X X
Show all the aqueous ionic compounds as the separate ions they really are.
Spectator ions just “watch the show” so we can remove them.
We are left with the net ionic equation
Cu(NO3)2(aq) + 2NaOH(aq)  Cu(OH)2(s) + 2NaNO3(aq)
Cu2+(aq) + 2NO3-(aq) + 2Na+(aq) + 2OH-(aq) 
Cu(OH)2(s) + 2Na+(aq) + 2NO3-(aq)
Net ionic: Cu2+(aq) + 2OH-(aq)  Cu(OH)2(s)
Only the aqueous compounds are separate ions so only they are written as ions. X X X X

6. Steps for a Net Ionic Equation
1. Get a balanced chemical equation.
2. Give the physical state of each compound. (s), (l), (g), or (aq)
3. Write the complete ionic equation, showing the dissociation of aqueous compounds
4. Cross out spectator ions.
5. Write net ionic equation

7. 2 Ag+1(aq) + 2 Cl-1(aq)  2 AgCl(s)
Practice Problem
Write the net ionic equation for:
MgCl2(aq) + 2AgNO3(aq)  2AgCl(s) Mg(NO3)2(aq)
2 Ag+1(aq) + 2 Cl-1(aq)  2 AgCl(s)

8. Practice Problem Write the net ionic equation for:
Mg(s) + NiSO4(aq)  Ni(s) + MgSO4(aq)
Mg(s) + Ni+2(aq)  Ni(s) + Mg+2(aq)